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Understanding Acids and Bases: Nomenclature, Properties, and Definitions

This comprehensive guide explores the essential concepts of acids and bases in chemistry. It covers acid nomenclature, including common acids like hydrochloric acid (HCl), sulfuric acid (H2SO4), and nitric acid (HNO3). Key properties of acids and bases are discussed, such as their tastes, reactions, and pH indicators. Definitions from various theories, including Arrhenius, Brønsted-Lowry, and Lewis, highlight the behavior of acids and bases. Additionally, distinctions between strong and weak electrolytes clarify their ionization in solutions. Perfect for students and chemistry enthusiasts!

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Understanding Acids and Bases: Nomenclature, Properties, and Definitions

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  1. Ch. 18 – Acids & Bases I. Introduction toAcids & Bases

  2. Review – Acid Nomenclature

  3. Review – Acid Nomenclature

  4. Review – Naming Acids • HCl • H2S • H2SO4 • H2SO3 • HNO3 • HNO2 • HBr • Hydrochloric acid • Hydrosulfuric acid • Sulfuric acid • Sulfurous acid • Nitric acid • Nitrous acid • Hydrobromic acid

  5. electrolytes electrolytes A. Properties ACIDS BASES • bitter taste • sour taste • turn litmus red • turn litmus blue • react with metals to form H2 gas • slippery feel • vinegar, milk, soda, apples, citrus fruits • ammonia, lye, antacid, baking soda

  6. HF H3PO4 H2SO4 B. Definitions • Monoprotic – an acid with one H+ • Polyprotic – an acid with more than one H+ • Diprotic – an acid with 2 H+ • Triprotic – an acid with 3 H+ monoprotic triprotic diprotic polyprotic

  7. H H – + O O Cl Cl H H H H B. Definitions • Arrhenius • Acids contain hydrogen • Acidsform hydronium ions (H3O+) in aqueous solution HCl+ H2O  H3O+ + Cl– acid

  8. B. Definitions • Arrhenius • Bases contain a hydroxide group • Bases form hydroxide ions (OH-) in aqueous solution H2O NaOH Na+ + OH- base

  9. conjugate base conjugate acid B. Definitions • Brønsted-Lowry • Acidsare proton (H+) donors • Bases are proton (H+) acceptors HCl + H2O  Cl– + H3O+ acid base

  10. conjugate base conjugate acid B. Definitions • Brønsted-Lowry • Conjugate Acidsare the result after a base accepts a hydrogen ion • Conjugate Bases are the result after an acid donates a hydrogen ion HBr + NaOH  NaBr + H2O acid base

  11. B. Definitions H2O + HNO3 H3O+ + NO3– B A CA CB H2O + NH3 NH4+ + OH- B CA CB A • Amphoteric – can be an acid or a base

  12. F - H2PO4- H2O HF H3PO4 H3O+ B. Definitions • Give the conjugate base for each of the following: • Polyprotic – an acid with more than one H+

  13. Br - HSO4- CO32- HBr H2SO4 HCO3- B. Definitions • Give the conjugate acid for each of the following:

  14. B. Definitions • Lewis • Acidsare electron pair acceptors • Bases are electron pair donors Lewis base Lewis acid

  15. - + C. Strength • Strong Acid/Base • 100% ionized in water • strong electrolyte NaOH KOH KOH RbOH CsOH Ca(OH)2 Ba(OH)2 HCl HNO3 H2SO4 HBr HI HClO4

  16. - + C. Strength • Weak Acid/Base • does not ionize completely • weak electrolyte HF CH3COOH H3PO4 H2CO3 HCN NH3

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